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Write Kc for each reaction, and find Δ n for each: (a) 4NH₃(g) + 5O₂(g) ⇌ 4NO(g) + 6H₂O(g); (b)…

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Write $K_c$ for each reaction, and find $\Delta n$ for each: (a) $4\text{NH}_3\text{(g)} + 5\text{O}_2\text{(g)} \rightleftharpoons 4\text{NO(g)} + 6\text{H}_2\text{O(g)}$ ; (b) $\text{CaCO}_3\text{(s)} \rightleftharpoons \text{CaO(s)} + \text{CO}_2\text{(g)}$ ; (c) $\text{H}_2\text{(g)} + \text{I}_2\text{(g)} \rightleftharpoons 2\text{HI(g)}$ .

Need a reminder? The key ideaShow

For $a\text{A} + b\text{B} \rightleftharpoons c\text{C} + d\text{D}$ : $K_c = \dfrac{[\text{C}]^c[\text{D}]^d}{[\text{A}]^a[\text{B}]^b}$ . $K_p = K_c(RT)^{\Delta n}$ with $R = 0.0831$ L bar K $^{-1}$ mol $^{-1}$ . Pure solids and liquids are left out. $Q_c < K_c$ : forward; $Q_c > K_c$ : backward. $\Delta G^\circ = -2.303\,RT\log K$ .

The worked solution

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Write Kc for each reaction, and find Δ n for each: (a) 4NH₃(g) + 5O₂(g) ⇌ 4NO(g) + 6H₂O(g); (b)…

The worked solution

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